Question

Why is dU (change in internal energy)= heat absorbed (Q[v])at constant Temperature and Volume.? And why is dH (enthalpy change)= heat change (Q[p]) at constant temperature and pressure? I do understand why constant pressure and volume is specified but why should the temperature be constant in both cases? shouldn't the first case imply dU=0 at constant temperature?

Answer 1

\[\Delta U=Q+W \]
\[W=0\]

Answer 2

W = -PΔV

Answer 3

I think we assume constant temperature so that we can calculate the total energy change without losing internal energy due to heat lost or gained.

Answer 4

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